Through stoichiometric calculations, the theoretical yield of indigo was calculated to be 1.70 g. However, when massed after the experiment, only 0.73 g of indigo had been produced.

What is the percent yield of indigo?

A) 97.0%
B) 232.8%
C) 57.1%
D) 42.9%

                     %age Yield  =  42.9 %

Explanation:

Percentage Yield is defined as the actual yield divided by theoretical yield. It is given as,

                   %age Yield  =  Actual Yield / Theoretical Yield × 100 --- (1)

Also,

         Actual Yield is the amount of desired product which is obtained after an experiment is completed. We can also call it the real yield which is obtained practically. While, theoretical yield is the yield which is calculated on paper. Hence, we can say that the actual yield is always less than theoretical yield due to many reasons including reaction conditions and researcher handling problems.

Thus we are given following data;

                   Theoretical Yield  =  1.70 g

                   Actual Yield  =  0.73 g

Putting these values in Eq. 1,

                   %age Yield  =  0.73 g / 1.70 g × 100

                   %age Yield  =  42.9 %

answer: your mm

explanation:

given:

mass of na = 115 g

excess cl2

to determine:

mass of nacl produced

explanation:

given reaction is-

2na(s) + cl2(g) → 2nacl(s)

since cl2 is in excess, na will be the limiting reagent

as per the reaction stoichiometry na: nacl = 1: 1

i.e. moles of na reacted = moles of nacl formed

now, # moles of na = mass of na/atomic mass

                                  = 115 g/23 g.mol-1 = 5 moles

therefore, moles of nacl = 5

molar mass of nacl = 58 g/mol

mass of nacl = 5 moles * 58 g.mol-1 = 290 g

ans: amount of nacl produced = 290 g